Consider the following reactions: CaSO4(s) Ca²+ + SO4²- CaF2(s) Ca²+ + 2F- Kso-10-4.59 Kso-10-10.3 a) What is the solubility of CaSO4(s) in water at 25 °C? b) What is the solubility of CaF2(s) in water at 25 °C? c) Will either of these two solids will precipitate if [F]=104 M, [SO4²-]-10-³ M and [Ca²+]=10¹² M?

Consider the following reactions: CaSO4(s) Ca²+ + SO4²- CaF2(s) Ca²+ + 2F- Kso-10-4.59 Kso-10-10.3 a) What is the solubility of CaSO4(s) in water at 25 °C? b) What is the solubility of CaF2(s) in water at 25 °C? c) Will either of these two solids will precipitate if [F]=104 M, [SO4²-]-10-³ M and [Ca²+]=10¹² M?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What is the solubility of MgCO3 in a solution that contains 0.090 M Mg²+ ions? (Ksp of MgCO3 is 3.5 x 10-⁹)
The Ksp of lead(II) carbonate, PbCO3, is 7.40 × 10-14. Calculate the molar solubility, S, of this compound. S = 2.72 X107 Incorrect M
Zinc hydroxide Zn(OH), has Ksp=4.5x10-17 In pure water calculate its małor solubility ?
In which solution is Fe(CIO4)3 most soluble? 0.400 M NaCl04 Pure water 0.200 M HC1 1.400 M Fe(NO3)3 1 x 10³ M NaOH The expression used to calculate the concentration of lead(IV) ions in a saturated solution of lead(IV) chloride is: (Ksp)l/5 None of these choices are correct. 4(Ksp)/4 (Ksp/256)/5 (Ksp/256) Which of the following compounds would supply the largest amount of Ag" in a 100 mL solution? O AgBrO3, Ksp = 5.38 x 10-5 AgCN, Ksp = 5.97 x 10-17 Ag2CrO4, Ksp = 1.12 x 10-12 O AgCl, Ksp = 1.6 x 10-10 O Ag2SO4, Ksp = 1.20 x 10-5 O O
What is the solubility of Mg(OH)2 at a pH of 11.10? (Ksp Mg(OH)2 is 1.6 × 10-1³)
What is the molar solubility (in mol L-1¹) of a salt with general molecular formula MX₂ (where M is a cation and X is an anion) in a solution already containing 0.513 mol L-¹ X-? The Ksp of MX₂ = 2.01 x 10-8
The Ksp of Ag2CO3 (MM = 275.81 g/mol) at 25°C is 8.1 x 10-12a. Calculate the molar solubility of Ag2CO3 at 25°C.b. What is the solubility of Ag2CO3 in mg/L?
In which solution will 0.0020 M AgNO3 form a precipitate? a 7.1x10-7 M NaBr (Ksp of AgBr=5.0x10-13) b 1.3x10-5M NaCl (Ksp of AgCl=1.8x10-10) c 4.2x10-14 M NaI (Ksp of AgI=8.3x10-17) d 7.4x10-7 M NaBrO4 (Ksp of AgBrO4=5.5x10-13)
At what molarity will 0.100 M Ca2+ begin to precipitate out of a solution of KAl(SO4)2?(Ksp of CaSO4=2.4x10-5) 2.4x10-4M KAl(SO4)2 4.9x10-3M KAl(SO4)2 2.4x10-3M KAl(SO4)2 1.2x10-4 M KAl(SO4)2
What is the ratio of SO42- to CO32- in a solution at equilibrium with both CaSO4 and CaCO3? (The solubility product of CaSO4 is 3.2 x 10-5).
Determine the molar solubility for BaCO3 (Ksp = 5.0 x 10 ^-9) in a solution that already contains 1.4 x 10 ^-4 M CO3 ions.
The molar solubility of palladium (II) thiocyanate at 25°C is 2.22 x 10-8 M. What is its Ksp value? The formula for palladium (II) thiocyanate is Pd(SCN)2. 4.38 x 10-23 4.93 x 10-16 2.22 x 10-8 1.09 x 10-23 6.56 x 10-30